\(5.1612 \mathrm{~g}\) of a metal is heated from \(294 \mathrm{~K}\) to \(574 \mathrm{~K}\) in a constant-pressure process. The melting point of metal is \(505 \mathrm{~K}\). We are given that

\[\begin{aligned} \text { Latent heat of fusion of the metal } & =14.5 \mathrm{cal} / \mathrm{g} \\ \text { Specific heat of solid metal } & =0.052 \\ \text { Specific heat of liquid metal } & =0.062 \end{aligned}\]

Calculate the change in entropy of the process.